Explain why the presence of a non volatile solute in solution reduces the tendency of the solvent molecule from escaping.

When 2.0 g of aspirin was shaken up in a flask containing two immiscible liquids it was found that the mole fractions in the two liqu ids were 0.11 and 0.18. When a further 1.0 g of aspirin was added, it was found that the mole fraction in the first liquid increased to 0.15. What would you expect the mole fraction in the second liquid to become?

(c) Are the strengths of the interactions between the particles in the solute and between the particles in the solvent before the solute and solvent are combined greater than, less than, or equal to the strengths of the interactions between solute particles and solvent particles after dissolution? Explain.

. a) The addition of 100 g of a compound to 750 g of CCl4 lowered the freezing point of the solvent by10.5 K. Calculate the molar mass of the compound. Kf = 30 K kg /molb) Explain why freezing point depression is observed when a non-volatile solute is dissolved in asolvent.

Given that the solubility of any organic material in a given solvent is due to the intermolecular forces present between the solvent and solute, solvents like hexanes (the alkanes isomers of C6H14) are rarely used for extraction purposes.  In the space provided here, suggest a reasonable explanation for this experimental observation.

For freezing point depression what is delta T mean? Is it the temperature of the solvent minus the temperature of the solution at freezing point?

Please order the following types of solute diffusivity from largest to smallest. D pore: Diffusivity of solute in a pore De: Effective diffusivity of solute through a heterogeneous membrane material DAB: Diffusivity of solute in water Dm :Diffusivity of solute through a membrane pore relative to the bulk concentration

14. 25.00 cm³ of 0.300 mol/dm³ sodium hydroxide solution is exactly neutralized by 0.100 mol/dm³ sulfuric acid. Calculate the volume of sulfuric acid needed in ml. Using dimensional analysis

A dilute solution of liquid X in liquid Y is prepared. It is found that the partial molar volume of liquid X is lower in the dilute solution than in its pure form, while the partial molar volume of liquid Y becomes larger. What molecular interpretations can you draw about the two liquids and the solution?

Solute S has a distribution constant of 4.9 between water (phase 1) and hexane (phase 2). A 89.0 mL solution of S in water is extracted five times with 14.0 mL of hexane. Calculate the fraction of S remaining in the aqueous phase. fraction remaining:

A CHM 126 student performed the "Determination of Molar Mass by Freezing Point Depression" experiment. He started the experiment by measuring the mass and freezing point of the pure solvent with minimal error. Instead of quickly finishing the experiment, he took a lunch break. After returning from lunch, he noted that the solvent had absorbed some impurities from the atmosphere. He went ahead and performed the rest of the experiment anyway. Assuming a negligible (very minor) change in the mass of the solvent after absorbing impurities, which of the following choices contains only correct statements: because of the experimental error, the measured ATwill increase, the measured molality will increase, and the measured molar mass will contain no additional error because of the experimental error, the measured ATwill decrease, the measured molality will decrease, and the measured molar mass will decrease because of the experimental error, the measured ATwill decrease, the measured molality…

5) The volume of several aqueous copper sulfate (CuSO4) solutions was precisely measured at SATP. All of the solutions were made by adding copper sulfate to 100.00 g of water. ncopper sulfate (mol) Vsolution (mL) 0 100.18 0.0330 100.16 0.0696 100.36 0.111 100.81 0.156 101.62 First, estimate the concentration-dependent partial molar volume of copper sulfate in water by taking finite differences. Second, fit the data to a hyperbola and take a derivative of the hyperbola to accurately calculate the partial molar volume of copper sulfate in water at each concentration. Interpret the partial molar volume at infinite dilution - what must copper sulfate be doing to the nearby water molecules?

the solubility of any organic material in a given solvent is due to the intermolecular forces present between the solvent and solute, hexanes (the alkanes isomers of C6H14) are rarely used for extraction purposes. What is a good reason for this experiment?

The mole fraction of CH3OH in an aqueous solution is 0.02 and density of solution 0.994 g cm-3 . Determine the molality and molarity.